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Ch.20 - Electrochemistry
Brown - Chemistry: The Central Science 14th Edition
Brown14th EditionChemistry: The Central ScienceISBN: 9780134414232Not the one you use?Change textbook
All textbooksBrown 14th EditionCh.20 - ElectrochemistryProblem 36a
Chapter 20, Problem 36a

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (a) Write the two half-cell reactions.

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Identify the oxidation and reduction components of the overall reaction. In this case, PdCl4^2- is reduced to Pd, and Cd is oxidized to Cd^2+.
Write the reduction half-reaction. Since PdCl4^2- is reduced to Pd, the palladium ion gains electrons. The equation will show the reduction of PdCl4^2- to Pd with the release of Cl^- ions.
Balance the reduction half-reaction for atoms other than hydrogen and oxygen. Ensure that the number of Pd and Cl atoms are equal on both sides of the equation.
Write the oxidation half-reaction. Since Cd is oxidized to Cd^2+, the cadmium metal loses electrons. The equation will show Cd transforming into Cd^2+.
Balance the oxidation half-reaction for atoms and charge. Ensure that the number of Cd atoms and the overall charge are equal on both sides of the equation.

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Key Concepts

Here are the essential concepts you must grasp in order to answer the question correctly.

Half-Cell Reactions

Half-cell reactions represent the oxidation and reduction processes occurring in a voltaic cell. Each half-cell reaction shows the transfer of electrons, with one species being oxidized (losing electrons) and another being reduced (gaining electrons). In the given reaction, identifying the species that undergo oxidation and reduction is essential for writing the half-cell reactions.
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Standard Cell Potential

The standard cell potential (E°) is the measure of the voltage produced by a voltaic cell under standard conditions (1 M concentration, 1 atm pressure, and 25°C). It indicates the driving force behind the electrochemical reaction, with positive values suggesting a spontaneous reaction. Understanding how to interpret and calculate standard cell potentials is crucial for analyzing the overall cell reaction.
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Electrochemical Series

The electrochemical series is a list of standard electrode potentials for various half-reactions, arranged from the most positive to the most negative. This series helps predict the direction of electron flow in a voltaic cell and the feasibility of reactions. By comparing the standard potentials of the half-reactions involved, one can determine which species will be oxidized and which will be reduced in the cell.
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Related Practice
Textbook Question

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (c) Sketch the voltaic cell, label the anode and cathode, and indicate the direction of electron flow

Textbook Question

(c) Why is it impossible to measure the standard reduction potential of a single half-reaction?

Textbook Question

Using standard reduction potentials (Appendix E), calculate the standard emf for each of the following reactions: (a) Cl21g2 + 2 I-1aq2 ¡ 2 Cl-1aq2 + I21s2

Textbook Question

A voltaic cell that uses the reaction PdCl42-(aq) + Cd(s) → Pd(s) + 4 Cl-(aq) + Cd2+(aq) has a measured standard cell potential of +1.03 V. (b) By using data from Appendix E, determine E°red for the reaction involving Pd.